The number of electrons transferred in a redox reaction directly affects the potential difference also known as the cell potential or electromotive force, EMF of the reaction. The relationship between the number of electrons transferred and the potential difference can be described using the Nernst equation.The Nernst equation is as follows:E_cell = E_cell - RT/nF * ln Q where:- E_cell is the cell potential potential difference at non-standard conditions- E_cell is the standard cell potential potential difference at standard conditions- R is the gas constant 8.314 J/molK - T is the temperature in Kelvin- n is the number of electrons transferred in the redox reaction- F is the Faraday constant 96,485 C/mol - ln Q is the natural logarithm of the reaction quotient, QAs the number of electrons n transferred in the redox reaction increases, the potential difference E_cell will also increase, assuming all other factors remain constant. This is because the term RT/nF in the Nernst equation will decrease as n increases, leading to a larger overall potential difference.In summary, the number of electrons transferred in a redox reaction directly influences the potential difference of the reaction. As the number of electrons transferred increases, the potential difference will also increase, provided all other factors remain constant.